F09_230_L08post - CHEM 230 F09 Lecture 8 Chapter 6:...

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CHEM 230 F09 Lecture 8 Chapter 6: Thermodynamics First Law Session ID: 230
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Outline Work Problem Measuring Enthalpy Heat exchange: Temperature change q = mC Δ T q A = -q B Phase change Δ H vap , Δ H fus Measure with calorimeter Reactions Themochemical equations (adding, reversing, stoichiometry) Hess’s Law Heats of formation
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Concept Question A gas is heated in a rigid container such that the internal energy of the gas increases, and the pressure in the vessel also increases. What is the sign of the enthalpy for this process? A. Positive B. Zero C. Negative D. Cannot be determined H = U + PV : enthalpy is defined for constant pressure only We cannot compute an enthalpy for a constant volume process (except in the special case where volume and pressure both constant, and Δ H = Δ U )
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One mole of a monoatomic ideal gas initially contained in a 5L vessel under a pressure of 10 bar at a temperature of 625K is carried through a cycle consisting of the following legs. What do you know about q, w, and Δ U? (a) an isothermal reversible expansion to a Fnal volume
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This note was uploaded on 03/29/2010 for the course CHEMISTRY 230 taught by Professor Gottfried during the Fall '10 term at University of Michigan.

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F09_230_L08post - CHEM 230 F09 Lecture 8 Chapter 6:...

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